chem 634 introduction to transition metal catalysis · basic organometallic mechanisms • to...

Chem 634

Introduction to Transition Metal Catalysis

Reading: Heg Ch 1–2 CS-B 7.1, 8.2–8.3, 11.3

Grossman Ch 6

Announcements

•  Problem Set 1 due Thurs, 9/24 at beginning of class

•  Office Hour: Wed, 10:30-12, 220 BRL

Announcements

Organometallic Complexes

M0 III IV V VI VII VIII IX X XI XII d3 d4 d5 d6 d7 d8 d9 d10 d10s1 d10s2

1st row Sc Ti V Cr Mn Fe Co Ni Cu Zn 2nd row Y Zr Nb Mo Tc Ru Rh Pd Ag Cd 3rd row La Hf Ta W Re Os Ir Pt Au Hg early dividing line late

Rh ClPPh3PPh3

Ph3PPPh3Pd PPh3PPh3 PPh3

ClPt

ClCl Cl

2–

Ootol2P N

IrB

CF3

CF3 4Ph

Ph2P

PPh2

RuNH2

H2N Ph

Ph

Cl

Cl

How Many Valence Electrons?

E

2s

2p x 3

LCAO's of 4 H 1s orbitals

C 4 x HCH4

Bonding orbitals filled...stable configuration.

Consider CH4… Recall the Octet Rule

How Many Valence Electrons? Transition metals have 5 d orbitals (plus s & 3 p’s)!

E(n+1)s

(n+1)p x 3

M LxMLx

Bonding and nonbonding orbitals filled...stable configuration.

nd x 5

x M–L bonding orbitals

(9–x) nonbonding orbitals

x M–L antibonding orbitals

Determining Electron Count of TM Complex

Ionic Method: All ligands are dissociated with their electrons.

L-type ligands = neutral, 2 e- donor X-type ligands = anionic 2 e- donor

M

X

L

X

L

n

M

X

X

LLn+y

where y = number of x-type ligands

M

X

L

X

L

mnemonic:

M+

X

L

X–

L

Electron counting is a formalism.

Example of Ionic Method Electron Counting

Fe2+

H–

C OFe COH

COOCOC

HCO

CO

CO

H–

4 X CO 4 X 2e- 8e-

2 X H– 2 X 2e- 4e- Fe(2+) (d6) 6e- ________________________________________

18e-

Note: Both Ionic and Neutral Methods give the same electron count, but differ in how they treat the metal center.

Charged Complexes

4 X Cl- 4 X 2e- 8e-

Pd(2+) (d8) 8e- ________________________________________

16e-

ClPdCl

ClCl

2– 2K+

Oxidation State

•  Formalism to account for “oxidation state” of metal center. •  This is only a formalism, in reality electrons (and thus charge) are

shared over both the ligand and metal. •  Nonetheless, oxidation state guides understanding of metal

reactivity. •  Using ionic method of electron counting arrives directly at metal

oxidation state. •  Example:

Fe COH

COOCOC

H

4 X CO 4 X 2e- 8e-

2 X H– 2 X 2e- 4e- Fe(2+) (d6) 6e- ________________________________________

18e-

Oxidation State = Fe(II)

Examples of X-type Ligands

hydride

halide

amido

alkoxide

M H

M Cl

H

Cl

M+ +

M+ +

M+ +

M+ +

-1

-1

-1

-1

2

2

2

2

M NR2

M OR

NR2

OR

alkyl

aryl (σ bound)

acetylide

silane

M+ +M CR3 CR3 -1 2

M M+ + -1 2

M R M+ + R -1 2

M SiR3 M+ + SiR3 -1 2

Ligand Complex Disconnection ligand e-ligand charge

Examples of X-type Ligands (More Complex)

acetate (η1)

acetate (η3)

allyl (η1)

allyl (η3)

M O

M

M

M

M+ +

M+ +

M+ +

M+ +


-1

-1

-1

-1

2

4

2

4

Me

O

O

OMe

O Me

O

OMe

O

cyclopentadienyl (Cp) M M+ + -1 6

•  𝜼 (eta) denotes “hapticity” = how many atoms of ligand are bond to metal from single donor site.

Examples of 2e– Donor “L”-type Ligands

phopshine

amine

carbonyl

alkene

sigma bond (C–H)

M PPh3

M NEt3

M C

M

MH

CR3

O

PPh3

NEt3

C O

H

CR3

M +

M +

M +

M +

M +


0

0

0

0

0

2

2

2

2

2

ether M OR2 OR2M + 0 2

sigma bond (H–H) MH

H

H

HM + 0 2

nitrile M N CR N CRM + 0 2

“L”-type Ligands Donating More than 2e–

•  𝜅 (kappa) denotes “denticity” = how many binding sites of a polydentate ligand are bound .


M

Mdiene

arene (η6)

arene (η2)

M

M +

M +

M +

0

0

0

4

6

2

MP

PPh Ph

Ph PhP

PPh Ph

Ph Ph

M +2 X 2e– L-type ligandsbisphosphine (κ2)

0 4

MP

NR R

R RN

NR R

R R

M +2 X 2e– L-type ligandsdiamine (κ2)

0 4

X2 Ligands

oxo M O M2+ +


-2 4O2-

imido (bent) M N M2+ + -2 4NR2-

triplet carbenes(alkylidines)

M CR2 M2+ + -2 4CR2

2-

R

NHC-Ligands

NNC

R

RM N

NCM

Sigma Bond Pi-Backbond


N-heterocyclic carbenesN

NM

R

R

N

N

R

R

M +0 2

18 Electron “Rule”

Many, but not all, stable, isolatable TM complexes are 18e– complexes.

NOTE: 18e– “rule” is more of a suggestion. Many of the most interesting, i.e. reactive, complexes do not follow this “rule”.

Pd

PPh3

PPh3Ph3P

PPh3

Pd = group 1010e- + 8e- = 18e-

Ru

Cl

Cl

H2N

NH2

Ph2P

PPh2

Ru = group 8+2 = d6

6+12 = 18

Basic Organometallic Mechanisms

•  To understand transition metal catalysis, we need to understand something about the mechanisms by which the catalysts operate.

•  Many TM catalyzed reactions proceed via a series of elementary steps.

Dissociative Ligand Substitution

common with: •  coordinately saturated •  18e- complexes

M

LL

LL

L

L

-LM

L

L

LL

L

L'M

LL

L'L

L

L

Associative Ligand Substitution

L'

L ML

LL'

L �L � M

L �

L �L �'L � M

L �

L �L �

common with: •  16 e- complexes •  requires open coordination site

Y* ML �

L �L

L'Y* M

L �L'

Ltrans effect

equatorial ligand w/strongest pi-interactions

Oxidative Addition

[Mn] RX

[Mn+2]R

X

•  formal oxidation state of metal center increases by two •  favored by electron-rich metal centers

Example:

Ph3P Pd0Ph3P

Ph

I

Ph3P PdIIPh3P

Ph

I

Reductive Elimination

[Mn]R

R[Mn-2] + R R

•  formal oxidation state of metal center decreases by two •  promoted by electron poor metal centers •  large ligands accelerate process •  microscopic reverse of oxidative addition

N

NNiII

Ph

NO

N

NNi0 +

O

NPh

Example:

Transmetallation

[Mn]R

X

M' R'[Mn]

R

R'+ M' X

•  Exchange of ligands between different metal centers •  No change in oxidation state at metals •  Exact mechanisms are complex, some are still unknown.

Ph3PPdII

Ph3P

Ph

IBu3Sn Ph Ph3P

PdIIPh3P

Ph

Ph+ Bu3SnI

Example:

Migratory Insertion

[Mn]R

X[Mn]

XR

•  Ligand inserts into adjacent metal-ligand bond •  No net change of oxidation state at the metal

Examples: PPh3

RhI

PPh3

OC CO

R

PPh3

RhI

PPh3

OCO

R

Ar

PdII

PPh3

Ph3P

+

PdII

PPh3

Ph3PAr

+

β-Elimination

[Mn]R [Mn]

R

•  Microscopic reverse of migratory insertion •  No net change of oxidation state at the metal •  Most often observed as β-hydride elimination from alkyl ligand •  Requires open coordination site on the metal center

PPh3

PdIIPh3P

+

Ar

Hnote opencoordination site

PPh3

PdII

H

Ph3P

+

Example:

β-Elimination

Ph

[Pd]H1H2

H3

H2

PhH3

Note: most of the time, β-hydride elimination is superfacial. This is because the mechanism is inner-sphere, involving formation of a metal-hydride bond.

PPh3

PdIIPh3P

+

Ar

Hnote opencoordination site

PPh3

PdII

H

Ph3P

+

α-Elimination

[Mn]R'H

R[Mn]

R

+ HR'

[Mn]R

R'

H

or: [Mn]

R' H

R ‡

Via:

not common in organic synthesis

Oxidative Coupling/Cyclization

[Mn] [Mn+2][Mn]

‡

σ−Bond Metathesis

[M] R R' R'' [M] R'+

R R''

[M] R

R' R''

‡ [M] R

R' R''

Via:

Common mechanism of C-H bond activation.

π−Bond Metathesis

[M] RX Y

[M] X R Y+

via:

[M] R

X Y

[M] R

X Y

[2+2] [retro 2+2] [M] R

X Y

Common in alkene metathesis.

chem 634 introduction to transition metal catalysis · basic organometallic mechanisms • to...

Documents